R3.2 Electron transfer reactionsIB Chemistry HL: Flashcards

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What is the oxidising agent in a redox reaction?

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What is the oxidising agent in a redox reaction?: The species that is reduced (gains electrons).
Balance: Cr₂O₇²⁻ → Cr³⁺ in acid.: Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O.
Sign of the anode in a voltaic cell?: Negative.
What does an electrolytic cell do?: Converts electrical energy into chemical energy, driving a non-spontaneous reaction.
Formula for E⦵cell?: E⦵cell = E⦵(cathode) − E⦵(anode).
What sign of E⦵cell shows a spontaneous reaction?: Positive.
Link between ΔG⦵ and E⦵cell?: ΔG⦵ = −nFE⦵cell.
A more negative E⦵ means the metal is…?: A stronger reducing agent (more easily oxidised).
Cathode product when aqueous KCl is electrolysed?: Hydrogen.
Anode product for concentrated NaCl(aq) with graphite?: Chlorine.
Anode product for dilute NaCl(aq) with graphite?: Mainly oxygen.
What happens at a copper anode in CuSO₄(aq)?: Cu → Cu²⁺ + 2e⁻ (the anode dissolves).
In electroplating, which electrode is the object?: The cathode.
Anode half-equation when silver plating with a silver anode?: Ag → Ag⁺ + e⁻.